C.P. Chemistry
Test Chapter 5
Study Guide
Chemical Names and Formulas
Ions and Ionic Compounds

Relate chemical bond formation to electron configuration.

Describe the formation of positive and negative ions.

Describe the formation of ionic bonds.

Account for many of the physical properties of an ionic compound.

Define anion and cation and infer charges on each.

Distinguish between ionic and molecular compounds.

Explain how all compounds obey the laws of definite and multiple
proportions.

Define polyatomic ion and know the most common symbols.

Write formulas for ionic compounds, molecular formulas, and acids.
C.P. Chemistry
Name___________________
Review Ch 5 Ionic Compounds/Chemical Names and Formulas
1. Write the noble gas configuration for the following elements and determine
how many valence electrons they have. Which one is not chemically
reactive? Why?
a. F
b. Ca
c. P
d. Ne
2. What is an anion? A cation? How do they form?
3. List the number of valence electrons for the following group. Then state
the type of ion the elements in each group would form. (ex.: Alkali metals
have 1 valence electron and form a +1 ion)
a. Group 1: Alkali metals
b. Group 2: Alkaline earth metals
c. Group 13: Boron family
d. Group 14: Carbon family
e. Group 15: Nitrogen
f. Group 16: Oxygen family
g. Group 17: Halogens
h. Group 18: Nobel gases
4. What type of ion would each of the following form?
a. An atom with 5 valence electrons
b. A halogen
c. An atom with atomic number 19
d. An atom with 2 valence electrons
e. An atom with 6 valence electrons
5. Write the full electron configuration for the following ions. Then write the noble
gas configuration. (Hint: Cations lose electrons from their s and p orbitals to form
ions.)
a. Fb. Ca2+
c. Ga3+
d. P2-
6. Do the nonmetals typically form anions or cations? Explain.
7.
Why do ionic compounds have high melting points?
8.
What is the difference between an ionic and a covalent bond?
9. Which monatomic ions required roman numerals? Why are they needed and what
do they mean?
10. Which ions use the "ide" ending? “ite?” “ate?”
11. What is the difference between a binary acid and an oxyacid?
12. What are the diatomic molecules?
13. State the law of definite proportions and the law of multiple proportions.
14. What does the chemical formula in an ionic compound represent? A molecular
compound?
15. How is a formula unit different from a molecule?
16. Molecular (Covalent) Compound Name
a.
Carbon dioxide
b.
Diphosphorus pentoxide
c.
Dinitrogen monoxide
Compound
Formula
d.
CCl4
e.
H2O
f.
SeF6
17.
Ionic Compound
Name
a.
magnesium nitrate
b.
iron (III) oxide
c.
sodium phosphide
d.
calcium phosphate
e.
titanium (II)
hydroxide
f.
lead (IV) chloride
Compound
Formula
g.
18.
Name or Formula Covalent
or Ionic
a.
CO
b.
Potassium nitrate
c.
CuSO4
d.
Sodium
bicarbonate
e.
P2O5
f.
Zinc nitrate
g.
Fe2O3
h.
Dihydrogen
monoxide
(NH4)3PO4
h.
V2O3
i.
SnCl2
j.
Ca(NO3)2
k.
CrSO4
19.
Acid Name
a.
Hydrochloric acid
b.
Chloric acid
c.
Sulfurous acid
Acid
Formula
d.
HF
e.
HNO3